Ask Question
11 May, 15:58

The value for Kw is 1.0 x 10-14 at 298K, but this value is temperature dependent. Given what you know about Kw and acid/base chemistry, what will the pH of water be at 283K if the value for Kw is 0.29 x 10-14? Is this solution acidic, basic, or neutral? A. pH = 7.26, acidicB. pH = 7.26, neutralC. pH = 7.00, neutralD. pH = 14.54, basicE. pH = 7.26, basic

+3
Answers (1)
  1. 11 May, 18:41
    0
    Water is a llittle basic solution at 283K, pH = 7.26

    Option E.

    Explanation:

    The water equilibrium is this:

    2H₂O → H₃O⁺ + OH⁻ Kw = 1x10⁻¹⁴

    At 283K, Kw = 0.29x10⁻¹⁴

    [H₃O⁺]. [OH⁻] = 0.29x10⁻¹⁴

    √0.29x10⁻¹⁴ = [H₃O⁺] → 5.38x10⁻⁸

    √0.29x10⁻¹⁴ = [OH⁻]

    - log [H₃O⁺] = pH

    - log 5.38x10⁻⁸ = 7.26

    pH > 7 = Basic

    pH < 7 = Acidic

    pH = 7 → Neutral
Know the Answer?
Not Sure About the Answer?
Find an answer to your question ✅ “The value for Kw is 1.0 x 10-14 at 298K, but this value is temperature dependent. Given what you know about Kw and acid/base chemistry, ...” in 📘 Chemistry if you're in doubt about the correctness of the answers or there's no answer, then try to use the smart search and find answers to the similar questions.
Search for Other Answers